Use the Bronsted-Lowry theory to explain (with examples) why water is amphoteric in acid-base reaction.

Explain the distinction between strong and weak versus concentrated and dilute acids. Include diagrams to represent these concepts.

The definitions below represent some of the emerging ideas by scientists reflecting on the chemistry of acids and bases.

Analyse and evaluate these definitions and make scientifically supported judgement about whether any parts of these definitions are satisfactory in the light of your knowledge.

The ${\mathrm{K}}_{\mathrm{w}}$ is a constant for the extent that pure water molecules dissociates into its component ions, protons $\left({\mathrm{H}}^{+}\left(\mathrm{aq}\right)\right)$ and hydroxide ions $\left({\mathrm{OH}}^{-}\left(\mathrm{aq}\right)\right)$. The ${\mathrm{K}}_{\mathrm{w}}$ value is the product of the hydrogen ion and hydroxide ion concentrations (or alternatively the square of the hydrogen ion concentration).

Table compares the extent that pure water molecules dissociates at different temperatures, and very precise measurements of pH values.

Describe the trends in the extent that water molecules in sample of water dissociate with an increase in temperature.

The ${\mathrm{K}}_{\mathrm{w}}$ is a constant for the extent that pure water molecules dissociates into its component ions, protons $\left({\mathrm{H}}^{+}\left(\mathrm{aq}\right)\right)$ and hydroxide ions $\left({\mathrm{OH}}^{-}\left(\mathrm{aq}\right)\right)$. The ${\mathrm{K}}_{\mathrm{w}}$ value is the product of the hydrogen ion and hydroxide ion concentrations (or alternatively the square of the hydrogen ion concentration).

Table compares the extent that pure water molecules dissociates at different temperatures, and very precise measurements of pH values.

Explain why the pH changes in response to the dissociation of water molecules. What does pH measure?